Concentration

• The more?concentrated?a solution is, the?greater?the number of?particles?in a given volume of solvent
• An increase in?concentration?causes in an increased?collision frequency?and therefore an increased?rate of reaction

The diagram shows a higher concentration of particles in (b) which means that there are more particles present in the same volume than (a) so the chances and frequency of collisions between reacting particles is increased causing an increased rate of reaction

Pressure

• An increase in pressure in reactions that involve gases has the same effect as an increased concentration of solutions
• When the?pressure?is increased, the molecules have less space in which they can move
• This means that the number of?effective collisions?increases due to an increased?collision frequency
• An increase in pressure therefore increases the?rate of reaction

The diagram shows a higher pressure in (b) which means that the same number of particles occupy a smaller volume, resulting in an increased collision frequency and therefore increased rate of reaction

• During a reaction, the?reactants?are used up and changed into the?products
• This means that as the reaction proceeds, the concentration of the reactants is?decreasing?and the concentration of the products is?increasing
• Because of this, the?rate of the reaction?is not the same throughout the reaction but?changes
• The rate of reaction during the reaction can be calculated from a?concentration-time graph.
• The?isomerisation of cyclopropane?to propene will be taken as an example:

Isomerisation of cyclopropane

• The concentrations of reactant (cyclopropane) and product (propene) over time can be experimentally obtained

Concentrations of cyclopropane & propene table

• When taking the measurements, the?temperature?should be kept the same at all times as a?change?in temperature will change the?rate of reaction
• A?concentration-time graph?for the?concentration of propene as well as cyclopropane?can be obtained from the above results
  • As an example, the concentration-time graph for propene is shown below:

The graph shows that the concentration of propene increases with time

Calculating the rate at the start of a reaction

• At the start of the reaction, the concentration-time curve looks almost linear
• The rate at this point can therefore be found by treating the curve as a linear line and by using:

• Using the graph, the average rate of the reaction over the first 5 minutes for propene is:

Line a shows the average rate over the first five minutes whereas line b shows the actual initial rate found by drawing a tangent at the start of the curve. The calculated rates are very similar for both methods

= 0.0009 mol dm^-3?s^-1

Calculating the rate as the reaction proceeds

• The curve becomes shallower with time which means that the rate decreases with time
• The rate of reaction can be calculated by taking short time intervals
• Eg. you can calculate the rate of reaction from 15 to 20 mins during which the concentration of propene increases from 0.68 to 0.83 mol dm-3:

= 0.0005 mol dm^-3 s^-1

• The smaller the time intervals, the more accurate the reaction rate value is
• Even more accurate is to find the rate of reaction at?different concentrations?of reactant or product at?particular time?points
• This can be done by drawing?tangents?at several points on the graph
  • As an example, the rates of reaction at different concentrations of cyclopropane are calculated by drawing the appropriate tangents:

The rate of reaction at 3 different concentrations of cyclopropane is calculated by drawing tangents at those points in the graph

Rate-concentration graph

• The calculated rates can then be summarised in a table to show how the rate of reaction changes with changing concentration of the reactants or products

Change in rate with decreasing concentration of cyclopropane table

• This data can then be used to plot a rate-concentration graph
• The graph shows that the rate is directly proportional to the concentration of cyclopropane
  • If you double the concentration of cyclopropane the rate of reaction will double too

The graph shows a directly proportional correlation between the concentration of cyclopropane and the rate of reaction